Across
- 1. The catalyst exists in a different phase than the reactants
- 3. A number, usually between 0 and 1, which represents the fraction of collisions with an orientation that allows the reaction to occur
- 5. Shows the relationship between the rate constant and the temperature in kelvin
- 6. Forms in one elementary step of a reaction mechanism and is consumed in another
- 7. The relationship between the rate of reaction and the concentration of the reaction
- 9. The reactant molecule in organic chemistry
- 10. A relationship between the concentration of the reactants and time. Depends on the order of the reaction
- 16. Biological catalyst that increases the rates of biochemical reactions. Usually large protein molecules with complex three-dimensional structures
- 18. A chemical reaction occurs after a sufficiently energetic collision between two reactant molecules
- 20. The time required for the concentration of a reactant to fall to one-half of its initial value
- 22. The rate of the reaction is directly proportional to the concentration of the reactant. Rate slows down as the reaction proceeds because the concentration of the reactant decreases
- 24. A substance not used up during a reaction, but increases the rate. It also does not affect the products obtained. Merely changes the pathway of the reactants to products and in doing so, reduces the activation energy and speeds up the reaction
- 26. A high-energy intermediate state that a molecule must go through to get from reactant to product
- 27. The series of individual chemical steps by which an overall chemical reaction occurs. A complete, detailed description of the reaction at the molecular level. Specifies the individual collisions and reactions that result in the overall reaction
- 28. The catalyst exists in the same phase or state as the reactants
Down
- 2. The rate of the reaction is proportional to the square of the concentration of the reactant. Thus rate is more sensitive to the reactant concentration
- 4. Change of concentration over change of time. Measure of how fast the reaction occurs
- 8. The sum of the reaction order exponents (m+n)
- 11. The slowest of the elementary steps, limits the overall rate of reaction and therefore determines the rate law for the overall reaction
- 12. Energy barrier or hump that must be surmounted for the reactants to be transformed into products
- 13. A number between 0 and 1 that represents the fraction of molecules that have enough energy to make it over the activation barrier on a given approach, resulting in a product. Increases with increasing temperature but decreases with increasing activation energy
- 14. The number of collisions that occur per unit time, which we can calculate for a gas-phase reaction from the pressure of the gasses and the temperature of the reaction mixture
- 15. The rate at any one point in time and represented by the instantaneous slope of the curve at that point. Determined by calculating the slope of the tangent to the curve at the point of interest
- 17. The rate of reaction is independent of the concentration of the reactant. Decreases linearly with time; rate is constant because reaction does not slow down as concentration of reactant decreases
- 19. The number of reactant particles involved in the step. Usually unimolecular and bimolecular, but on rare occasions termolecular
- 21. Specific area on the enzyme's structure that the substrate connects into like a lock
- 23. The number of approaches to the activation barrier per unit time. Equal to orientation factor times collision frequency
- 25. A singular step in a reaction mechanism that cannot be broken down into simpler steps